Top topic this week
Back to FAQs
Related FAQs
Frequently Asked Question
Questions asked by users might not always be phrased in the clearest way.
Deduce the relationship between kp and kc for the gaseous equilibria; (i) $2no_{(g)}+o_{2}(g)rightarrow 2no_{2}(g)$ (5 marks)
Accepted Answer
The relationship between Kp and Kc for the given gaseous equilibrium can be deduced using the following equation:
Kp = Kc(RT)^Δn
Where:
Kp is the equilibrium constant in terms of partial pressures.
Kc is the equilibrium constant in terms of molar concentrations.
R is the ideal gas constant (0.0821 L atm/mol K).
T is the temperature in Kelvin.
Δn is the change in the number of moles of gas in the balanced chemical equation (moles of products - moles of reactants).
For the reaction:
2NO(g) + O2(g) ⇌ 2NO2(g)
Δn = (2) - (2 + 1) = -1
Therefore, the relationship between Kp and Kc is:
Kp = Kc(RT)^-1
Kp = Kc/(RT)
Articles you might like